Trent Nettles Daisy Benitez Martha Nochez Introduction: In the Stoichiometry: Can You Make 2.00 Grams of a Compound? lab, what is first required as a basic procedure is predicting the chemical reactions of your given pair of reactants, balancing the equation of your reactants and products, and finally calculating the molar mass of each individual compound. The two compounds, once combined, should result in a compound close to 2.00 grams.
Procedure: 1) Writing the balanced equation. In the products side, H2O is included. The precipitate that was concluded was CaCO2 in the calcium acetate monohydrate and sodium carbonate reaction to form calcium carbonate and sodium acetate. The way that the products were formed was considered by the solubility rules. The mass of how much of the product would form of each of the reactants was calculated using different conversion factors. The moles of one substance from the balanced equation to moles of the precipitate. Then the grams were calculated using the molar mass(grams per mole). 2) Take the graduated cylinder and pour 50 mL of water twice for both of the reactants. The water must be distilled so the product will have no impurities. 3) Measure the exact amounts to get 2.00g of our substance. 4) The grams of the reactants is put into a 250 mL beaker, 5) The water is then poured into the beaker. 6) The water is mixed in well with the reactants 7) The filter paper must then be measured using a scale, before weighing the products. 8) Place the filter paper in filter/funnel. 9) The solutions are then poured into one beaker to form our product. 10) Put the product into the filter and wait for the residue. 11) Carefully take out the finished substance.
The mixture of the reactants Calcium Acetate Monohydrate and Sodium Carbonate.
To filter out both of the products, a filter along with filter paper to collect the precipitate was used and a beaker to collect the waste product. Before we filtered our paper, we premeasured the paper and tared it in order to obtain a more accurate result. When we measured the filter paper, we collected the precipitant as the other product was being filtered into a beaker.
Materials
Filter paper (1.57g)
Calcium acetate monohydrate (3.52 g)
Sodium carbonate (2.47g)
2 paper cups
Beakers (250 mL)
2 Graduated cylinders (100 mL)
2 Pipets
2 Scales
Funnel
Ring stand
(2) 50 mL of water
Claim: The solution containing our precipitate contained impurities due to errors committed in experimental design and human error.
Results: One must take into consideration human error and experimental flaws when the experiment was conducted. The actual end product was 2.76g of the precipitate. The percent yield was 138% . Those conclusions were formed because the number of moles taken were taken from the balanced equation of the molar mass of both substances. The actual end product was 2.76g of the precipitate. Since no reaction is going to be perfect when done by humans, the outcome was incorrect but not far off.
The filtration of our mixture with the use of a funnel.
Conclusion:
The solution containing our precipitate contained impurities due to errors committed in experimental design and human error. Our reasoning behind the lab resulting in 2.76 grams was the fact that our group committed a few slight errors in regards to experimental design and human error. Our lab used two different scales, one with two places after the decimal and the other a mere one decimal place. which is an error in experimental design. This may have caused us to make inaccurate measurements. The lab also experienced human error when the filter paper was damaged and ripped in the process of filtering the mixture produced from the two reactants. Although we may have gone over 2.0 grams, specifically 2.57 grams, and our percent yield was higher than expected (138%), another source of impurities was when we dropped the end product before weighing it. What could be done so this problem wont occur again is to make sure our lab equipment is thoroughly clean. What also could be done is to handle materials and equipment with care, so none of the products would be lost. Along with care, staying consistant with the materials being used should be done.
Daisy Benitez
Martha Nochez
Introduction:
In the Stoichiometry: Can You Make 2.00 Grams of a Compound? lab, what is first required as a basic procedure is predicting the chemical reactions of your given pair of reactants, balancing the equation of your reactants and products, and finally calculating the molar mass of each individual compound. The two compounds, once combined, should result in a compound close to 2.00 grams.
Procedure:
1) Writing the balanced equation. In the products side, H2O is included. The precipitate that was concluded was CaCO2 in the calcium acetate monohydrate and sodium carbonate reaction to form calcium carbonate and sodium acetate. The way that the products were formed was considered by the solubility rules. The mass of how much of the product would form of each of the reactants was calculated using different conversion factors. The moles of one substance from the balanced equation to moles of the precipitate. Then the grams were calculated using the molar mass(grams per mole).
2) Take the graduated cylinder and pour 50 mL of water twice for both of the reactants. The water must be distilled so the product will have no impurities.
3) Measure the exact amounts to get 2.00g of our substance.
4) The grams of the reactants is put into a 250 mL beaker,
5) The water is then poured into the beaker.
6) The water is mixed in well with the reactants
7) The filter paper must then be measured using a scale, before weighing the products.
8) Place the filter paper in filter/funnel.
9) The solutions are then poured into one beaker to form our product.
10) Put the product into the filter and wait for the residue.
11) Carefully take out the finished substance.
To filter out both of the products, a filter along with filter paper to collect the precipitate was used and a beaker to collect the waste product. Before we filtered our paper, we premeasured the paper and tared it in order to obtain a more accurate result. When we measured the filter paper, we collected the precipitant as the other product was being filtered into a beaker.
Materials
Claim:
The solution containing our precipitate contained impurities due to errors committed in experimental design and human error.
Results:
One must take into consideration human error and experimental flaws when the experiment was conducted. The actual end product was 2.76g of the precipitate. The percent yield was 138% . Those conclusions were formed because the number of moles taken were taken from the balanced equation of the molar mass of both substances. The actual end product was 2.76g of the precipitate. Since no reaction is going to be perfect when done by humans, the outcome was incorrect but not far off.
Conclusion:
The solution containing our precipitate contained impurities due to errors committed in experimental design and human error. Our reasoning behind the lab resulting in 2.76 grams was the fact that our group committed a few slight errors in regards to experimental design and human error. Our lab used two different scales, one with two places after the decimal and the other a mere one decimal place. which is an error in experimental design. This may have caused us to make inaccurate measurements. The lab also experienced human error when the filter paper was damaged and ripped in the process of filtering the mixture produced from the two reactants. Although we may have gone over 2.0 grams, specifically 2.57 grams, and our percent yield was higher than expected (138%), another source of impurities was when we dropped the end product before weighing it. What could be done so this problem wont occur again is to make sure our lab equipment is thoroughly clean. What also could be done is to handle materials and equipment with care, so none of the products would be lost. Along with care, staying consistant with the materials being used should be done.